Which statement accurately describes the distance between gas molecules?

The correct statement indicates that, on average, gas molecules are very far apart. This is a fundamental characteristic of gases in contrast to solids and liquids. In a gas, the molecules move freely and are not held together by strong intermolecular forces, leading to large spaces between them. This high degree of separation allows gas molecules to fill the volume of their container, and their movement is largely independent of one another.

The behavior of gas molecules can be described by the concepts of kinetic molecular theory, which reinforces that gas particles are in constant motion and that their average distance from one another is significantly greater than in liquids or solids. The vast distances between molecules result in gases having low densities and the ability to expand and compress significantly.

In contrast, the other statements do not accurately capture the properties of gas molecules. Molecules being very close together or in contact with one another misrepresents the nature of gases, as they do not exhibit a fixed structure unlike solids. Additionally, while it is true that under certain conditions, such as changes in temperature or pressure, the distances between gas molecules might vary, on average, they are still considerably far apart, making the first two options inaccurate descriptions of gas behavior.